The document discusses key concepts in material technology including: 1. It defines the basic structure of atoms and different types of materials including elements, mixtures, and compounds. 2. It describes atomic structure including atomic number, atomic mass, and atomic orbits. The periodic table is introduced as a way to classify and understand elements and their properties. 3. Different types of crystal structures are defined including body centered cubic, face centered cubic, and hexagonal close packed. Bonding types such as covalent, metallic, and ionic are also introduced. 4. Terminology used in phase diagrams is defined including phases, equilibrium, composition, liquidus, and solidus. Binary alloy systems containing two components are also

1. JF302 – Material Technology 1 1.0 MATERIAL STRUCTURE AND BINARY ALLOY SYSTEM

2. 1.1 Material structure and element periodical table EPT

3. 1.1.1 The terminology of: Atom Consist primarily three basic subatomic particles:- protons, neutrons and electrons. Basic unit of matter that consist of a dense; solid, liquid and vapour. Contains central nucleus surrounded by a cloud of negatively charged electrons. b. Element Chemical substance consisting of one type of atom distinguished by its atomic number. Eg:O 2 , H 2 , CL 2 and N 2 .

4. 1.1.1 The terminology of: c. Mixture The molecules of two or more different substances are mixed in the form of alloys, solutions, suspension and colloids. A material system made up by two or more different substance which are mixed together but are not combined chemically. d. Compound Chemical substance consisting of two or more different chemical elements that can be separated into simpler substance by chemical reaction. Eg; H 2 O and HCl

5. 1.1.2 Atomic numbers and atomic mass of EPT. Atomic numbers The number of proton (positively charged particles) that arc in its nucleus. In a neutral atom the atomic number = to the number of electrons in its charge cloud. b. Atomic masses Relative atomic mass of an alement in the mass in grams of 6.023x10 23 atoms (Avogadro’s number,N A ) of the element.

6. 1.2 Atomic Numbers, Atomic Masses and Atomic Orbits 1. Atomic Numbers Neutral atom = numbers of proton = numbers of electron 2. Atomic Masses and Atomic Weight Atomic Weight = Atomic masses of element/Atomic masses of Hydrogen Atomic Masses = atomic numbers = number of proton + number of neutron 3. Atomic Orbits Using the 2n2 formula to state the total of atoms in every orbit, where n is total of orbit 1st orbit, n = 1 Total of atom = 2 (1)2 = 2 2nd orbit, n = 2 Total of atom = 2 (2)2 = 8

7. 1.1.3 Total number of atomic orbits Symbol Atomic number Atomic mass Table 1.1.3: Maximum number of electrons for each principal atomic shell

8. Example: Potassium with atomic number 19; the orbital should be:

9. 1.3 Periodic Table of the Elements 1. It is a chart of list of elements which all the elements with same chemical properties in one line as one group. 2. The horizontal rows of elements on the periodic table called periods. The vertical columns called groups or families . 3. Characteristics : i. 18 lines of boxes in vertical, 7 lines of boxes in horizontal ii. 8 groups start with group I until VIII iii. arrange by atomic number start with Hydrogen iv. elements in same line horizontally has same total of orbits v. chemical properties of an atom depend on total of valency atom vi. when electron are followed from group I to group III, metal properties of an element become lessen but total of electron will increase and become the non-metal properties vii. elements in group I has 1 electron in outer orbit, elements in group II has 2 electron in outer orbit viii. each period has same total of orbits

10. 4. Usages : i. to classified certain elements easier ii. as a revision where elements reactive properties can be known (way to the right, the reactive properties are lessen) iii. elements in first group has same chemical properties iv. easier to acknowledge certain unknown element and also its properties and the usage v. easier to analyze and understand every reaction between the elements

11. 1.4 Crystal Structures It is atomic arrangements which have a repetitive pattern in all the three dimensions of space are called crystal structures or crystals. Fig 1 : Structure and grain boundaries

12. 2. There are 4 types well-known crystal structures and it was : (i) simple cube

13. (ii) body centered cubic/ BCC

14. (iii) face centered cubic/ FCC

15. (iv) hexagonal close packed/ HCP

16. 1.5 Types of Bonding 1.5.1 Covalent Bonding Occurs when two atoms (same elements) have a tendency to accept electrons which are satisfied for both by sharing the electron valency. Cl2 molecules. Couple of sharing electrons

17. 1.5.2 Metallic Bonding Occurs when two metal atoms have a tendency to give up their electrons and shared with all atoms close to them and formed of an electron cloud that spreads throughout the solid metal.

18. 1.5.3 Ionic / Electrovalence Bonding Exists between two unlike atoms that had a strong tendency to give up electrons (a metal), close to an atom that has a strong tendency to accept electrons (a nonmetal) and allows a transfer of one or more electrons depending on the valence of the atoms an example is natrium chloride (NaCl) Before After electron transferred from natrium to chlorine Na Cl 2.8.1 2.8.7

19. 1.6 The Stages Of Grain Structures Formation 1. Solidification process occurs along with the grain formation. 2. Nucleus tips freely find their own way to much colder place. 3. Causing the nucleus to grow and expanding. 4. The expand will form the secondary dendrite arm with 90 degree to each other. 5. This will continue until a structure called dendrite structure existed.

20. Fig 2:The Stages Of Grain Structures Formation

21. 1.7 The Differences Between Base Metal and Alloy 1. Base metal metal has same elements, extreme properties and cannot fulfill the need for engineering work. its characteristics : (i) malleable – can be shape to many form (ii) ductile – can be form to fine wire 2. Alloy a metal alloy is a combination of two or more metals or a metal and a non-metals.

22. 1.8 Types Of Solid Solutions Disordered Solid Solution Solute and solvent atoms are randomly distributed on lattice sites Solute atoms Solvent atoms

23. Ordered Solid Solution The atoms (solute and solvent) take up preferred positions and the solution becomes ordered Solute atoms Solvent atoms

24. Interstitial Solid Solution Atoms of small atomic radius fit into the empty spaces or interstices of the lattice structure of the solvent atoms Solute atoms Solvent atoms

25. Intermetallic Compounds made up of 2 or more elements producing a new phase with its own composition, crystal structure and properties Intermetallic compound (valence compound) is a phase, having chemical composition equal to a fixed simple ratio, like CuZn,Cu 3 Sn, Mg 2 Pb, etc. Sometimes intermetallic compounds exist over a range of composition, differing from the valence law. Intermetallic compounds of this sort are called electron compounds or intermediate solutions . An example of a phase diagram with intermetallic compound AB 2 is shown in the figure below.

26. 1.9 Terminologies In Phase Diagram 1. Phase Is a region that differs in structure or composition from another region 2. Equilibrium Phase Diagram Are graphical representations of what phases are present in a materials system at various temperatures, pressures and compositions 3. Composition Are percentage of certain materials contains purposely or not added to another material. With this it can cause changes in phases, the properties and the shape of the microstructures. 4. Liquidus The temperature at which liquid starts to solidify under equilibrium conditions. 5. Solidus The temperature which all liquid has completely solidified.

27. 1.10 Binary Alloy System 1. Binary phase diagram is a phase diagram in which there are only two components and a mixture of two metals (a binary alloy).